Question

1.50 moles of N2 at 825 mmHg and 303 K are contained in a 34.3 L bottle. What is the pressure of the system if an additional 1.00 mole of gas is added to the bottle and the temperature is reduced to 273 K?

Answer 1

1240.8964 mmHg

Step-by-step explanation:

I believe you only need to use
`PV = nRT` for this problem.

P = Pressure in mmHg

V = Volume in Liters

n = Number of Moles

R = Gas Constant in mmHg/1mol

T = Temperature in Kelvin

Since you start with 1.50 moles of N2 and add an additional mole of N2, you will have 2.50 moles of N2.

Assuming that the volume of the bottle does not change,

P(34.3) = (2.5)(62.363)(273)

Note that 62.363mmHg/1mol is the gas constant R.

P = ((2.5)(62.363)(273))/(34.3) = 1240.8964 mmHg (approximately)

Hope this helps!